1.2 10-2 M H2Te Chem 210 Final: Mastering Chem Flashcards | Quizlet Q: The acid dissociation . Kb = 1.80 10?9 . Calculate the value of (H3O+) in a 0.01 M HOBr solution. HI Posterior Thigh _____ 4. 1.2 10^-6 spontaneous Q < Ksp Pure water, 0.10 M potassium chromate is slowly added to a solution containing 0.50 M AgNO3 and 0.50 M Ba(NO3)2. 2003-2023 Chegg Inc. All rights reserved. No effect will be observed since C is not included in the equilibrium expression. Pyridine, C5H5N, has Kb = 1.7 x 10-9 and reacts with water as C5H5N + H2O arrow C5H5NH+ + OH-. 2 7.41 Which acid, if any, is a strong acid? H2O2(aq) If Ka = 1.5 x 10^-7 for this reaction, what is the pH of a 0.3 M solution of H2S? H2O = 2, Cl- = 2 1. B. acid dissociation C. base dissociation D. self-ionization 3. Get control of 2022! The pH of a 0.010 M aqueous weak acid solution is 6.20 at 25 degrees Celsius. H2C2O4 = 1, H2O = 4 2.223 Ar > HF > N2H4 Contact. Enough of a monoprotic acid is dissolved in water to produce a 0.0138 M solution. A galvanic cell consists of one half-cell that contains Ag(s) and Ag+(aq), and one half-cell that contains Cu(s) and Cu2+(aq). The K value for the reaction is extremely small. Ar > N2H4 > HF A- HA H3O+ 1.03 103 yr, The reaction shown below occurs in the blood between hemoglobin (Hb) and oxygen. What is n for the following equation in relating Kc to Kp? Your email address will not be published. HCl, Identify the strongest acid. NH3 and, Give the characteristics of a strong acid. Solved Write The Balanced Equation For Ionization Of Weak Base Pyridine C5h5nc5h5n In Water H2oh2o Phases Are Optional I M Putting This Answer And It Says Is Wrong. Titanium carbide is an alloy of titanium (r = 215 pm) containing 20% carbon by mass (r = 170 pm). 0.031 M. The equilibrium constant is equal to 5.00 at 1300 K for the reaction: The reaction will shift to the left in the direction of reactants. at T > 298 K 1.94. Solution Containing a Conjugate Pair (Buffer) 2. What is the conjugate base of acetic acid and what is its base dissociation constant? N2H4 > HF > Ar, Estimate Grxn for the following reaction at 850 K. networking atomic solid What is the hydronium ion concentration and the pH for an aqueous solution of NH3 that has a hydroxide ion concentration of 2.25 10-3 M? CO2(g) + C(graphite) 2 CO(g) You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Seattle, Washington(WA), 98106. 3 Cl2(g) + 2 Fe(s) 6 Cl-(aq) + 2 Fe3+(aq) What are the difficulties in developing perennial crops? Ag+(aq) + e- Ag(s) E = +0.80 V B) 0. Draw up an ICE table for the reaction of 0.150 M formic acid with water. Breaks in this system of automatic functions can cause dissociation symptoms. The entropy of a gas is greater than the entropy of a liquid. All of the above processes have a S > 0. Mn(s) olyatomic A and D only 8.9 10-18 Acetic acid is a weak monoprotic acid and the equilibrium . Learn about three popular scientific definitions of acids and bases. Work Plz. The Kb for pyridine is 1.7 x 10^ -9. pH = ________________ (please show work when possible). Free atoms have greater entropy than molecules. nonspontaneous, A hot drink cooling to room temperature. write the balanced equation for the ionization of the weak base pyridine, C5H5N, in water 5 Answers There is no word like addressal. 2.1 10-2 Pyridine is a weak base with the formula C5H5N. What effect will increasing the temperature have on the system? Pyridinium chloride. From the following chemical reactions determine the relative Brnsted-Lowry acid strengths (strongest to weakest). Strong Acid + Strong Base B. b) Calculate the equilibrium concentrations of H_3O^+, OCN^-, and HOCN. 1. Lemon juice is a weak acid. It has a [H+] of 5.0 10^-2 - BRAINLY A: Click to see the answer. Rn Problem 8-24. What is the Ag+ concentration when BaCrO4 just starts to precipitate? Calculate Ka for HOCN. Calculate Kb for the base. Chemical Equation For The Ionization Of Pyridine C5h5n In Water Calculate the pH of a 0.065 M C5H5N (pyridine) solution. If 11.3 grams of sample of pyridine is dissolved in 250.0 mL of water, what are the equilibrium concentration of all species present?2. What is the pH of a 0.375 M solution of HF? CO32- PbSO4, Ksp = 1.82 10-8 H2C2O4 = 3, H2O = 2, Balance the following reaction under basic conditions. (Kb = 1.7 x 10-9), Calculate the pH of a 0.053 M pyridine solution at 25 degrees Celsius. Become a Study.com member to unlock this answer! None of the above statements are true. Q > Ksp Cd2+(aq) Cl2(aq) + Br2(l) BrO3-(aq) + Cl-(aq) 10.68 -1, Consider the following generic reaction for which Kp = 5.51 105 at 25C: all of the above, Which of the following acids will have the strongest conjugate base? Since you know that, #color(purple)(|bar(ul(color(white)(a/a)color(black)("1 L" = 10^3"mL")color(white)(a/a)|)))#, you can say that this sample will be equivalent to, #1 color(red)(cancel(color(black)("L"))) * (10^3"mL")/(1color(red)(cancel(color(black)("L")))) = 10^3"mL"#, #10^3color(red)(cancel(color(black)("mL"))) * "1 g"/(1color(red)(cancel(color(black)("mL")))) = 10^3"g"#, The solution is said to be #0.800%# by mass pyridine and #0.990%# by mass pyridinium chloride. Zn +48.0 kJ HA H3O+ A- Ecell is negative and Grxn is positive. H, What element is being oxidized in the following redox reaction? \(K_a\) is an acid dissociation constant, also known as the acid ionization constant. Determine the Ka for CH3NH3+ at 25C. molecular solid P(O2) = 0.41 atm, P(O3) = 5.2 atm Sin. Calculate the pH of a solution that is 5.91 x 10-2 M in HF and 2.99 x 10-1 M in the salt LiF? Study with Quizlet and memorize flashcards containing terms like _____ is found in carbonated beverages due to the reaction of carbon dioxide with water. acidic, 2.41 10^-10 M, Which of the following solutions would be classified as acidic? SO3(g) 1/2 O2(g) + SO2(g) Kc = ? The equation for the dissociation of pyridine is C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq). What can you conclude about Ecell and Ecell? 1.209 104 yr Determine the value of the missing equilibrium constant. Q: Draw the mechanism of the E2 Reaction with an Alkyl Halide. P4O10(s) P4(s) + 5 O2(g) When we add HF to H2O the HF will dissociate and break into H+ and F-. Determine the molar solubility of MgCO3 in pure water. (Kb = 1.7 x 10-9), Determine the pOH of a 0.382 M C5H5N solution at 25 degrees Celsius. b) Write the equilibrium constant expression for the base dissociation of HONH_2. The pH of 0.050 M cyanic acid, HOCN(aq), is 2.38. a) Write the hydrolysis reaction for this acid. CH4(g) + H2O(g) CO(g) + 3 H2(g) This system has appreciable quantities of both pyridine (Py) and pyridinium chloride. 2 at T < 298 K (Kb = 1.7 x 10-9), Calculate the H3O+ in a 0.045 M HOCl solution. pH will be equal to 7 at the equivalence point. No precipitate will form at any concentration of sulfide ion. 5.11 10-12 2) A certain weak base has a Kb of 8.10 *. Hydrogen ions cause the F0 portion of ATP synthase to spin. Ka of HF = 3.5 104. 3 Cl2(g) + 2 Fe(s) 6 Cl-(aq) + 2 Fe3+(aq) ClO(g) + O3(g) Cl(g) + 2 O2(g) Grxn = ? If the ionization constant of water, Kw, at 40C is 2.92 10-14, then what is the hydronium ion concentration for a neutral solution? Determine the pH of a 0.324 M C5H5N solution at 25 degrees Celsius. Chem 2 Chapter 15 Flashcards | Quizlet For noble gasses, entropy increases with size. Its asking to determine if its acidic or base. PDF diSSociation conStantS of organic acidS and BaSeS - St. Olaf College +1.40 V, Which of the following is the strongest reducing agent? . Set up an ice table for the following reaction. 353 pm Contain Anions and Cations 1.3 10^3 Which two factors must be equal when a chemical reaction reaches equilibrium? 2.23, Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25C. Acid/Base Equilibria- Chapter 16 | PDF | Acid | Ph At what concentration of sulfide ion will a precipitate begin to form? No effect will be observed. Answered: Pyridine, C5H5N, is a toxic, | bartleby :1021159 . 1. A solution that is 0.10 M HCN and 0.10 M LiC, Which of the following solutions is a good buffer system? O NH4NO3 You may feel disconnected from your thoughts, feelings, memories, and surroundings. Acid with values less than one are considered weak. The relative abundance, for electrons of 72 volts energy, and the appearance potential are given for each ion. Q: a. CHCHCHCH-Br b. C. 4. (c) Which of these two substances is a stronger base? Homework 2 with Answer - Broward College, South Campus Homework 2 CHM 3.558 of pyridine is Catalytic sites in the F1 portion of ATP synthase phosphorylate ADP. Ne The value of an acid dissociation constant for the pyridinium ion, which is a pyridine's conjugate acid is 7.14x10. 2 NaH(s) + H2O(l) 2 NaOH + H2(g) Why is my internet redirecting to gslbeacon.ligit.com and how do I STOP THIS. We know from our chemistry classes that: The base-dissociation constant, kb, for pyridine, c5h5n, is 1.4x10-9 the acid-dissociation constant, ka, for the pyridinium ion, (pyridine's conjugate acid, is __________. 2.20 C5H5N(aq) + H2O(l) C5H5NH+(aq) + OH-(aq), What are the Brnsted-Lowry acids in the following chemical reaction? Acid dissociation constant will be calculated as: Kw = Ka Kb, where. +1.01 V, A voltaic cell is constructed with two silver-silver chloride electrodes, where the half-reaction is Medium. 1 answer. H3O+, Which Brnsted-Lowry acid is not considered to be a strong acid in water? Write the equilibrium constant K for CH3COOH + H2O = H3O^ + + CH3COO^ What are the conjugate acid-base pairs in the following chemical reaction? 4 Entropy is an extensive property. A written paragraph su metallic atomic solid, Identify the type of solid for ice. (Solved) - 91) What is the pH of a 0.30 M pyridine solution that has a You can ask a new question or browse more college chemistry questions. Xe, Which of the following is the most likely to have the lowest melting point? Dihydrogen phosphate H 2PO 4 -, has an acid NaOH + NH4Cl NH3 +H2O+NaCl. Question1 pOH=1/2pKb-1/2logC=1/2(-log1.9*10-9)-1/2log(1.2)=1/2(8.7)-1/2(0.08)=4.35-0.04=4.31 So, pH=14-pOH=14-4.31=9.69 Thus 3rd option(9.68) is the correct answer. phase separation We can write a table to help us define the equation we need to solve. 39.7 donates more than one proton. Calculate the pH for an aqueous solution of acetic acid that contains 2.15 10-3 M hydronium ion. Which of the following represents a conjugate acid-base pair? (Ka = 1.52 x 10-5). A: The dissociation constant or ionization constant (Ka) of an acid indicates the strength of acids. Which of the following can be classified as a weak base? 5.6 10^-10, All of the above will form basic solutions, Which one of the following will form a basic solution in water? NaOH, HBr, NaCH3CO2, KBr, NH4Br. 1 3.25 10-4 M, Determine the molar solubility of Fe(OH)2 in pure water. K(l) and Br2(g) Fe3+(aq) | Fe(s) || Cl-(aq) | Cl2(g) | Pt 2.44 10-17 M, The molar solubility of CuI is 2.26 10-6 M in pure water. The pH at 25 degrees Celsius of an aqueous solution of the sodium salt of hydrocyanic acid (NaCN) is 11.05. 2Al(s) + 3I2(s) 2AI3+(aq) + 6I-(aq) Calculating Equilibrium Concentrations - Chemistry LibreTexts C3H8O2(aq) + KMnO4(aq) C3H2O4K2(aq) + MnO2(s) 1, Part A Part complete The reaction is spontaneous ________. Identify the statement that is FALSE. Answered: The base-dissociation constant, Kb, for | bartleby to the empployees was very informative. +656 kJ Ka = (Kw/Kb). Q Ksp Presence of acid rain The acid dissociation constant for this monoprotic acid is 6.5 10-5. (Use H3O+ instead of H+. (b) % ionization. HCN(aq) + H2O(l) H3O+(aq) + CN-(aq). HF N2H4 Ar A solution that is 0.10 M HCN and 0.10 M LiCN The equation for ionization is as follows. RbI HClO4 47 CH3CO2H(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq). What is the equilibrium constant expression (Ka) for the acid dissociation of hydrocyanic acid HCN? Entropy generally increases with increasing molecular complexity. Given that at 25.0 degree C Ka for HCN is 4.9 * 10-10 and Kb for NH3 is 1.8 * 10-5, calculate Kb for CN- and Ka for NH4+. Fe Which set of coefficients, when used in the order listed, will balance the following skeleton equation for the combustion of benzene, C6H6(l)? Therefore answer written by Alex 29 A certain acidic vitamin is essential for all mammals since it plays a role in mineral absorption. The value of an acid dissociation constant for the pyridinium ion, which is a pyridine's conjugate acid is 7.14x10.. How we calculate acid dissociation constant? Assume that H and S do not vary with temperature. A) hydrofluoric acid with Ka = 3.5 10-4. ( ECA5, p.187) Calculate the pH and fraction of dissociation of (a) 10 2.00 M and (b) 10 10.00 M barbituric acid. Ksp for Fe(OH)2= 4.87 10-17. 1.37 10^9 American chemist G.N. Justify your answer. National Institutes of Health. If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral? The reaction will shift to the left in the direction of reactants. Q: Write the equilibrium-constant expressions and obtain numerical values for each constant in. A bu er is prepared that is 0.100 M in phenylamine and 0.200 M in phenylammonium cation (C 6H 5NH + 3). At equilibrium, the H+ in a 0.280 M solution of an unknown acid is 4.12 x 10-3 M. Determine the degree of ionization of this acid. Entropy increases with dissolution. (Ka = 4.9 x 10-10). B only Given that the pH for acetic acid is 2.41, the Ka = 1.8 10-5 and assuming the density of vinegar to be 1.00 g/cm3, what is the percent dissociation of acetic acid in vinegar? B and C only subtitutional Write a balanced base ionization reaction for methylamine (CH3NH2) in water. Diaphragm _____ 3. b.) NH4+ and OH increased hardness, CHEM: ADVANCED EQUILIBRIUM DYNAMIC STUDY MODU, CHEM: INTEGRATED RATE LAWS & ARRHENIUS EQUATI, CHEM: RATE PF REACTION & RATE LAW STUDY MODULE. The base is followed by its Kb value. ________ + HSO3- ________ + H2SO3. HF(aq) arrow F-(aq) + H+(aq); Ka = 6.80 x 10-4, Determine the pH of a 0.62 M NH4NO3 solution at 25 deg C. The Kb for NH3 is 1.76 x 10^-5. The acid dissociation constant, Ka for the Pyridium ion or the conjugate acid of Pyridine is to be determined. (PDF) Initial Reaction of Hexachlorodisilane on Amorphous Silica 0.0750 M Cu 4.17 [HCHO2] < [NaCHO2] 1. HX is a weak acid that reacts with water according to the following equation. Which metal could you use to reduce Cr3+ ions but not Mn2+ ions? 1. Ssurr = +321 J/K, it is not possible to predict the spontaneity of this reaction without more information. C7H15NH2. If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral? The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity. Write the equilibrium expression and calculate the value of Ka f. The ionization constant for hypochlorous acid (HClO) is K_a= 2.8 times 10^{-8} at T= 25 degrees C. Find the pH for an aqueous solution that is 0.0500 M in HClO. (Ka = 1.8 x 10-4). Pyridine, {eq}C_5H_5N 1.35 10^7 Ecell is positive and Ecell is negative. Metalloid Using the basic dissociation constant formula, the dissociation expression is Kb=[C5H5NH+][OH-][C5H5N] K b = [ C 5 H 5 N H + ] [ O H - ] [ C 5 H 5 N . interstitial, increased density 8 The equation for the dissociation of NH3 is Which will enhance the formation of rust? Answered: The reaction HCO3 CO2+ H is an | bartleby 2.3 10^-11 In order to be able to use the Henderson - Hasselbalch equation, which for a buffer that contains a weak base and its conjugate looks like this What is the % ionization in a 3.0 M solution? thank you. You can ask a new question or browse more Chemistry questions. (Ka = 2.9 x 10-8). sorry for so many questions. The properties listed above that would apply to (NH4)2CO3 would be what (eq. C 3 Answers C5H5N in water > C5H5NH+ & OH- Kb = [C5H5NH+] [OH-] / [C5H5N] 1.5e-9 = [x] 1. 10.68 4.32 9.68 8.72 What is the hydronium ion concentration of an acid. (a) Write the balanced chemical equation for this acid-base reaction, identifying the conjugate acid/base pairs. H2S The pH of the resulting solution is 2.61. A tablet containing 500.0 mg of aspirin (acetylsalicylic acid or HC9H7O4) was dissolved in enough water to make 100 mL of solution. In order to be able to use the Henderson - Hasselbalch equation, which for a buffer that contains a weak base and its conjugate looks like this, #color(blue)(|bar(ul(color(white)(a/a)"pOH" = pK_b + log((["conjugate acid"])/(["weak base"]))color(white)(a/a)|)))#, you will need to determine the concentrations of pyridine and of the pyridium cation. Pentagonal-bipyramidal WF5(NC5H5)2 was isolated and characterised by X-ray crystallography and . 0.016 M HA (aq) + H_2O (l) to H_3O^+ (aq) + A^- (aq) If the starting concentration of HA a 1.00 times 10^{-3} M solution has a pH = 6.53, determine the K_a for the acid. Calculate the pH of the solution made by adding 0.50 mol of HOBr and 0.30 mol of to 1.00 L of water. potassium iodide dissolves in pure water Now, the problem doesn't provide you with the density of the solution; however, because you're dealing with such small amounts of pyridine and pyridinium chloride, you can assume that the density of the solution is approximately equal to that of water. As we already know, strong acids completely dissociate, whereas weak acids only partially dissociate. b. Part A-Using K, to Calculate OH What is the pH of a 0.65 M solution of pyridine, C5H5N? If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system is View Available Hint(s) PDF AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) - College Board Calculate the pH of a 0.10 M solution of pyridine (C5H5N; Kb = 1.7 10^-9): asked Jul 30, 2019 in Chemistry by Satkriti (69.5k points) acids; bases; 0 votes. 2.10 not at equilibrium and will shift to the right to achieve an equilibrium state. Loading. No creo que Susana _____ (seguir) sobre los consejos de su mdico. Solved What is the pH of a 1.2 M pyridine solution that - Chegg The equation for the dissociation Which of the following solutions has the highest concentration of hydroxide ions [OH-]? What effect will increasing the pressure of the reaction mixture have on the system? This observation can be explained by the net ionic equation Nothing will happen since calcium oxalate is extremely soluble. C6H5NH + HOH ==> C6H5NH2^+ + OH^-, C5H5N(aq) + H2O(l) <------> C5H5NH+(aq) + Calculate the value of Ka for chlorous acid at this temperature. What is its atomic radius? PDF Chemistry 192 Problem Set 5 Spring, 2019 Solutions write the balanced equation for the ionization of the weak base Ssys>0 +332 kJ The standard emf for the cell using the overall cell reaction below is +2.20 V: We reviewed their content and use your feedback to keep the quality high. Acid dissociation constant will be calculated as:Kw = Ka Kb, where, Kw = dissociation constant of water = 10, Kb = base dissociation constant for pyridine = 1.4 10, Ka is an acid dissociation constant will be calculated as:Ka = Kw / Kb, On putting these values on the above equation, we get:Ka = 10 / 1.4 10, To know more about acid dissociation constant, visit the below link:brainly.com/question/26998, This site is using cookies under cookie policy . Identity. (b) Calculate the ratio of [C5H5N]/[C5H5NH+] if the solution has a pH of. Pyridine C5H5N is a weak base with Kb=1.7x10^-9. What is - Study.com Xe, Part A - Either orPart complete Pt, Fe(s) | Fe3+(aq) || Cl2(g) | Cl-(aq) | Pt, Determine the cell notation for the redox reaction given below. What is the % of ionization if a 0.114 M solution of this acid? HF > N2H4 > Ar (1) What is the [OH-] (molarity) of a 0.1660 M piperidine? 11.777 We are given the base dissociation constant, Kb, for Pyridine (C5H5N) which is 1.4x10^-9. (b) What must be the focal length and radius of curvature of this mirror? The Kb for pyridine is 1.7 x 10 ^-9 Enter your answer in the . Grxn = 0 at equilibrium. Determine for a 0.25 M pyridine (Kb = 1.7 * 10-9): (a) pH (b) % ionization. Calculate the H3O+ in a 1.4 M solution of hypobromous acid. The acetate ion, is the conjugate base of acetic acid, CH 3 CO 2 H, and so its base ionization (or base hydrolysis) reaction is represented by. What is the conjugate What is the conjugate acid of ammonia and what is its Al(s), Which of the following is the strongest oxidizing agent? C1=CC= [NH+]C=C1. Enter the Kb value for CN- followed by the Ka value for NH4+, separated b, What is the pH of an aqueous 0.032 M pyridine, (C5H5N)? The concentrations of chloride ion in the two compartments are 0.0222 M and 2.22 M, respectively. Nothing will happen since Ksp > Q for all possible precipitants. OPUS (Open ULeth Scholarship)Browsing Wetmore, Stacey by Author 1.7 10^2 min lithium fluoride forms from its elements neutral HBr(sol) + CH3COOH(sol) CH3C(OH)2+(sol) + Br-(sol) and more. H2O = 2, Cl- = 5 Ksp (MgCO3) = 6.82 10-6. pH will be greater than 7 at the equivalence point. K = [P4O10]/[P4][O2]^1/5 a.) (THE ONE WITH THE TABLE). 1): C5H5N(aq) + H2O(l) = OH-(aq) + C5H5NH+(aq) Nothing will happen since Ksp > Q for all possible precipitants. The equilibrium constant will increase. Determine the Kb of a base at 25 degrees Celsius if a 0.02 M aqueous solution of the base has a pH of 7.60 (this implies that it is an equilibrium pH). Nov 29, 2019 is the correct one. Ecell is positive and Grxn is negative. the F- will grab an H+ from C5H5NH+ making the weak acid HF and C5H5N, Kb C5H5N = 1.710^-9 so, Ka C5H5N = 5.8810^-6, Your email address will not be published. What effect will increasing the volume of the reaction mixture have on the system? 3. 3 O2(g) 2 O3(g) G = +326 kJ K = [O2]^-5 The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity. A 0.125-M aqueous solution of C5H5N (pyridine) has a pH of 9.14. 1. equilibrium reaction [HCHO2] > [NaCHO2] Which acid solution has the lowest pH? Calculate the K_a for the acid. K = [P4O10]/[P4][O2]^5, Express the equilibrium constant for the following reaction. The. (Hint: Calculate Ka. I2(s), Ag(s) is formed at the cathode, and Cu2+(aq) is formed at the anode. What is the pH of a 0.15 molar solution of this acid? The following pictures represent aqueous solutions of three acids HA (A = X, Y, or Z); water molecules have been omitted for clarity. A)4.9 10-24 B)2.0 10-5 C)2.0 109 D)4.0 . Calculate the pH of the solution.
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